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4.5 L of Mg(OH)2 solution was titrated with 5.03 mL of 0.200 M HCl. Calculate the the molarity of Mg(OH)2 solution and the ksp.
What should be the infusion rate in mL per hour. With a drop factor of 10 drops per mL, calculate the infusion in drops per minute.
What about the molecule as a whole? Is that molecule CH4 a polar or non-polar?
if 0.91 mol of cs2 reacts with oxygen completely according to the equation cs2l 3 o2g rarr co2g 2 so2g what volume
A block of metal has a width of 3.2 cm, a length of 17.1 cm, and height of 5.7cm. Its mass is 1.2kg. Calculate the density of the metal.
Calculate the percentages of dissociated and undissociated forms present in the following solutions:
Calculate how many whole drops (.05 mL/drop) of 6 M HCl are required to dissolve this. (I found this to be 11.59 drops
fe2o3 2al -----gt 2fe al2o3what masses of ironiii oxide and aluminum must be used to produce 15.0 g of iron? what is
Compute the concentration of IO3- in a 5.92 mM Pb(NO3)2 solution saturated with Pb(IO3)2. The Ksp of Pb(IO3)2 is 2.5 × 10-13. Presume that Pb(IO3)2 is a negligible source of Pb2 compared to Pb(NO3)2.
The half-equivalence point of a titration occurs half way to the end point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.560 moles of a monoprotic weak acid
4Au + 8KCN + O2 + 2 H2O --> 4 KAu(CN)2 + 4 KOH what is the minimum amount of KCN (in g) needed to react with 15.6 g of gold?
Explain most natural bodies of water have a ph range of 6-9. Explain what species are the dominant contributors to alkalinity. Utilize a speciation diagram and one or more PKa values to explain.
An excess of aqueous silver nitrate, AgNO3 was added to precipitate the bromide ion as silver bromide. If 8.00g of the soluble salt produced 2.00g of silver bromide, what was the mass percentage of the chloride in the sample?
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